Boiling Point of Organic Compounds

This organic chemistry video tutorial provides a basic introduction into boiling point of organic compounds such as straight chain alkanes, branched alkanes, aldehydes, amines, alcohols, and alkyl halides. It explains why polar molecules usually have a higher boiling point that nonpolar molecules based on intermolecular forces such as hydrogen bonding, dipole dipole interactions, and hydrogen bonds.
Organic Chemistry - Basic Introduction:
• Organic Chemistry - Ba...
Acids and Bases - Basic Intro:
• Acids and Bases - Basi...
Resonance Structures:
• Resonance Structures
IUPAC Nomenclature of Alkanes:
• IUPAC Nomenclature of ...
Van Der Waal Forces:
• Van Der Waals Forces
_______________________________
Boiling Point - Test Question:
• Boiling Points of Alkanes
Melting Points of Alkanes:
• Melting Points of Alkanes
Physical Properties of Alkanes:
• Physical Properties of...
Water Solubility of Vitamins:
• Water Solubility of Vi...
_______________________________
Homolytic & Heterolytic Cleavages:
• Homolytic and Heteroly...
Newman Projections:
• Newman Projections
Organic Chemistry PDF Worksheets:
www.video-tuto...
Organic Chemistry Exam 1 Playlist:
bit.ly/3kJnNXU
Full-Length Videos and Worksheets:
/ collections

[@TheOrganicChemistryTutor]

Organic Chemistry PDF Worksheets: www.video-tutor.net/orgo-chem.html Full-Length Exams and Worksheets: www.patreon.com/MathScienceTutor/collections Next Video: kzbin.info/www/bejne/jYmpq596d7uSobs Newman Projections - Full 59 Minute Video: bit.ly/3itPNy2

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So basically the more hydrocarbons an alkane group has the higher the boiling point.

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[@lovejilly7]

Hello, when we are comparing organic compounds with halogens, you said that bigger atoms would result in higher boiling points because of the increased London dispersion forces. Does this mean that the effect of the halogen's electronegativity is negligible? I thought that the one with fluorine would have a higher boiling point than the one with bromine because fluorine is more electronegative and would cause a greater dipole moment.

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[@happydoppyzsay]

I think that since dipole dipole interaction is stronger than Vander Waals interaction, the boiling point should be decreasing in the order of F --> Cl --> Br --> I.

[@mamadoualieujallow1354]

thats right but here he is taking the size of the atom first before considering the electronegativity reason being similar to resonance structure. the charge of the anion is more stable to chlorine than fluorine tho fluorine is more electronegative but chlorine is larger and can stabilize the charge more than the fluorine. i hope that helps?

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He said that electron cloud of Bigger atom will spread more due to which the interaction between the molecules increases

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[@abrehamephrem1302]

In the comparison between ethyl chloride and ethyl bromide, wouldn't the polarity of Cl be considered??

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14:30 also, look at the structure of primary amine, it’s linear!

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[@ThriveNow123]

Arent there hydrogen bonds @4:08 as well? Between Hydrogen and Oxygen?

[@Sanyakhan803]

No because H is not directly attached to O. There not a high dipole in C-H bonds.

[@ThriveNow123]

@@Sanyakhan803 so does that mean that for an h-bond to occur, there must always be an intramolecular force between hydrogen and Nitrogen, Oxygen or fluorine?

[@Sanyakhan803]

@@ThriveNow123 if there is a O-H, N-H etc bond IN a molecule, there is hydrogen bonding between molecules. For example in an aldehyde, -CHO, oxygen isnt bonded to hydrogen. So there is no hydrogen bonds. Hydrogen bonds exist when there is a large dipole only.

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@@ThriveNow123 And yes, hydrogen bonds only occur in between two molecules, between O/N/F and H.

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plz plz also make a video on topic:-MELTING POINT and also include SYMMETRICAL PACKING concept of determining melting point...

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to see how big an atom is, do we look at the atomic number or the radius? The radius can be lower for heavier atoms relative to a atom with lower atomic number

[@emmalee2122]

At 12:15, doesn't NH2 provide 2 H-bonding sites? Wouldn't this result in more H-bonds in a mixture and therefore a higher boiling point than for the compound with the singe -OH hydrogen bonding site? I understand that electronegativity plays a role, but isn't having 2 H-bonds also a significant factor?

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In amines there aren't 2 H bonding sites, only one of them undergoes H bonding, and hence electronegativity plays a vital role.

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Can u explain what happens in primary, secondary and tertiary aniline?

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[@marcoantoniolopezdelapuent5559]

Great! For those studying hydrocarbon Alkanes specifically, you only have to count the number of bonds.

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[@muhammadafiq4403]

why primary alcohol has higher b.p than primary amine? I thought amine would have higher b.p since it has 2 H which can form lot more hydrogen bond compared to primary alcohol.

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[@flyingthundergod3999]

Cl is more electronegative than Br but for one example we didn't use electronegativity but used atom size to compare?

[@flyingthundergod3999]

Bcz they are halogen?

[@shantanusingh6433]

at 12:31 there are 2 h bond in NH2 but why it has less b.p?

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both water and amine have 3 h bonds each.coz no of h = lone pairs+no of h atom attached to F or O or N.so we have to compare polarity of bond for further confirmation.

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Does a higher boiling point mean a molecule is more stable?

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why does butene have a lower boiling point than butane?

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What is the atomic mass of boron from the atomic boiling point of carbon?

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[@amazingannyoing1716]

I'm a bit confused Doesn't fluorine have a greater electronegativity so it can create a dipole dipole interaction that is much stronger than the other halogens in methyl alkines, hence is it supposed to have a greater bp?

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how about the boiling point of alcohols which the OH in different carbon?

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